Textbook-Integrated Guide to Educational Resources

TIGER

A New "Bottom-Up" Framework for Teaching Chemical BondingTami Levy Nahum, Rachel Mamlok-Naaman, Avi Hofstein, and Leeor KronikThis article presents a general framework for bonding that can be presented at different levels of sophistication depending on the student's level and needs. The pedagogical strategy for teaching this model is a "bottom-up" one, starting with basic principles and ending with specific properties.Levy Nahum, Tami; Mamlok-Naaman, Rachel; Hofstein, Avi; Kronik, Leeor. J. Chem. Educ.2008, 85, 1680.

Atomic Properties / Structure |

Covalent Bonding |

Ionic Bonding |

Lewis Structures |

Materials Science |

MO Theory |

Noncovalent Interactions

More on ClO and Related RadicalsWilliam B. JensenThe novel Lewis structure for the ClO radical and other related 13e isoelectronic species presented by Hirsch and Kobrak is identical to that proposed by Linnett over 40 years ago for the same species on the basis of his well-known double-quartet approach to Lewis structures.Jensen, William B. J. Chem. Educ.2008, 85, 783.

Ionic Bonding |

Lewis Structures |

Free Radicals

Lewis Structure Representation of Free Radicals Similar to ClOWarren Hirsch and Mark KobrakAn unconventional Lewis structure is proposed to explain the properties of the free radical ClO and a series of its isoelectronic analogues, particularly trends in the spin density of these species. Hirsch, Warren; Kobrak, Mark. J. Chem. Educ.2007, 84, 1360.

Atmospheric Chemistry |

Computational Chemistry |

Covalent Bonding |

Free Radicals |

Lewis Structures |

Molecular Modeling |

MO Theory |

Valence Bond Theory

The Mechanism of Covalent Bonding: Analysis within the Hückel Model of Electronic StructureSture Nordholm, Andreas Bäck, and George B. BacskayHckel molecular orbital theory is shown to be uniquely useful in understanding and interpreting the mechanism of covalent bonding. Using the Hckel model it can be demonstrated that the dynamical character of the molecular orbitals is related simultaneously to the covalent bonding mechanism and to the degree of delocalization of the electron dynamics. Nordholm, Sture; Bäck, Andreas; Bacskay, George B. J. Chem. Educ.2007, 84, 1201.

Let Us Give Lewis Acid–Base Theory the Priority It DeservesAlan A. ShafferThe Lewis concept is simple yet powerful in its scope, and can be used to help beginning students understand reaction mechanisms more fully. However, traditional approaches to acid-base reactions at the introductory level ignores Lewis acid-base theory completely, focusing instead on proton transfer described by the Br?nsted-Lowry concept.Shaffer, Alan A. J. Chem. Educ.2006, 83, 1746.

More on the Nature of ResonanceRobert C. KerberThe author continues to find the use of delocalization preferable to resonance. Kerber, Robert C. . J. Chem. Educ.2006, 83, 1291.

Aromatic Compounds |

Covalent Bonding |

Molecular Properties / Structure |

Resonance Theory |

Nomenclature / Units / Symbols

More on the Nature of ResonanceWilliam B. JensenSupplements a recent article on the interpretation of resonance theory with three additional observationsone historical and two conceptual.Jensen, William B. J. Chem. Educ.2006, 83, 1290.

If It's Resonance, What Is Resonating?Robert C. KerberThis article reviews the origin of the terminology associated with the use of more than one Lewis-type structure to describe delocalized bonding in molecules and how the original usage has evolved to reduce confusionKerber, Robert C. . J. Chem. Educ.2006, 83, 223.

Valence, Covalence, Hypervalence, Oxidation State, and Coordination NumberDerek W. SmithIt is argued that the terms valence, covalence, hypervalence, oxidation state, and coordination number are often confused and misused in the literature. It is recommended that use of the term valence, and its associated terminology, should be restricted to simple molecular main group substances and to some oxoacids and derivatives, but avoided in both main group and transition element coordination chemistry. Smith, Derek W. J. Chem. Educ.2005, 82, 1202.

Electronegativity and the Bond TriangleTerry L. Meek and Leah D. GarnerThe dependence of bond type on two parameters, electronegativity difference (??) and average electronegativity (?av), is examined. It is demonstrated that ionic character is governed by the partial charges of the bonded atoms, and metallic character by the HOMOLUMO band gap.Meek, Terry L.; Garner, Leah D. J. Chem. Educ.2005, 82, 325.

Atomic Properties / Structure |

Covalent Bonding |

Metallic Bonding |

Ionic Bonding |

Main-Group Elements

Exothermic Bond Breaking: A Persistent MisconceptionWilliam C. GalleySurveys taken the past several years at the onset of an introductory physical chemistry course reveal that the vast majority of students believe that bond breaking is exothermic.Galley, William C. J. Chem. Educ.2004, 81, 523.

Covalent Bonding |

Calorimetry / Thermochemistry

Teaching Molecular Geometry with the VSEPR ModelRonald J. GillespieThe difficulties associated with the usual treatment of the VB and MO theories in connection with molecular geometry in beginning courses are discussed. It is recommended that the VB and MO theories should be presented only after the VSEPR model either in the general chemistry course or in a following course, particularly in the case of the MO theory, which is not really necessary for the first-year course. Gillespie, Ronald J. J. Chem. Educ.2004, 81, 298.

How We Teach Molecular Structure to FreshmenMichael O. HurstExamination of how textbooks discuss various aspects of molecular structure; conclusion that much of general chemistry is taught the way it is for historical and not pedagogical reasons.Hurst, Michael O. J. Chem. Educ.2002, 79, 763.

An Investigation of the Value of Using Concept Maps in General ChemistryGayle Nicoll, Joseph S. Francisco, and Mary B. NakhlehStudy of the degree to which students in introductory chemistry classes linked related concepts; comparisons of a class in which concept mapping was used and another in which it was not.Nicoll, Gayle; Francisco, Joseph S.; Nakhleh, Mary B. J. Chem. Educ.2001, 78, 1111.

Covalent Bonding |

Learning Theories

Lewis Structures in General Chemistry: Agreement between Electron Density Calculations and Lewis StructuresGordon H. PurserThe internuclear electron densities of a series of X-O bonds (where X = P, S, or Cl) are calculated using quantum mechanics and compared to Lewis structures for which the formal charges have been minimized; a direct relationship is found between the internuclear electron density and the bond order predicted from Lewis structures in which formal charges are minimized.Purser, Gordon H. J. Chem. Educ.2001, 78, 981.

Fast Ionic Migration of Copper ChromateAdolf CortelAmong the many demonstrations of ionic migration in an electric field, the ones showing the migration of colored Cu+2 and CrO4-2 ions are popular. The demonstration described here introduces some modifications to allow a fast displacement of these ions.Cortel, Adolf. J. Chem. Educ.2001, 78, 207.

A Comment on Molecular Geometry Frank J. GombaA method of determining the correct molecular geometry of simple molecules and ions with one central atom is proposed. While the usual method of determining the molecular geometry involves first drawing the Lewis structure, this method can be used without doing so. In fact, the Lewis structure need not be drawn at all. The Lewis structure may be drawn as the final step, with the geometry of the simple molecule or ion already established.Gomba, Frank J. J. Chem. Educ.1999, 76, 1732.

Covalent Bonding |

Molecular Properties / Structure |

VSEPR Theory

The Use of Molecular Modeling and VSEPR Theory in the Undergraduate Curriculum to Predict the Three-Dimensional Structure of MoleculesBrian W. Pfennig and Richard L. FrockDespite the simplicity and elegance of the VSEPR model, however, students often have difficulty visualizing the three-dimensional shapes of molecules and learning the more subtle features of the model, such as the bond length and bond angle deviations from ideal geometry that accompany the presence of lone pair or multiple bond domains or that result from differences in the electronegativity of the bonded atoms, partial charges and molecular dipole moments, and site preferences in the trigonal bipyramidal electron geometry. Pfennig, Brian W.; Frock, Richard L. J. Chem. Educ.1999, 76, 1018.

Molecular Modeling |

Molecular Properties / Structure |

Covalent Bonding |

VSEPR Theory

Lewis Structures Are Models for Predicting Molecular Structure, Not Electronic StructureGordon H. PurserThis article argues against a close relationship between Lewis dot structures and electron structure obtained from quantum mechanical calculations. Lewis structures are a powerful tool for structure prediction, though they are classical models of bonding and do not predict electronic structure. Purser, Gordon H. J. Chem. Educ.1999, 76, 1013.

Molecular Properties / Structure |

Covalent Bonding |

Computational Chemistry |

Quantum Chemistry |

MO Theory |

Learning Theories |

Lewis Structures |

Molecular Modeling

A Way To Predict the Relative Stabilities of Structural IsomersJohn M. LyonThis paper discusses a method to evaluate the relative stabilities of structural isomers of inorganic and organic compounds. The method uses a simple set of rules that can be applied with only a knowledge of the electron configuration of the atoms and the periodic trends in atomic size.Lyon, John M. J. Chem. Educ.1999, 76, 364.

Covalent Bonding |

Diastereomers |

Molecular Properties / Structure

The Gravity of the SituationDamon DiementeThis article presents a few calculations demonstrating that gravitational attraction between atoms is many orders of magnitude weaker than the gravitational attraction between Earth and an atom, and that the gravitational attraction between two ions is many orders of magnitude weaker than the electromagnetic attraction between them. Diemente, Damon. J. Chem. Educ.1999, 76, 55.

Atomic Properties / Structure |

Covalent Bonding |

Noncovalent Interactions

An Alternative Framework for Chemical BondingWilliam R. RobinsonRecent, qualitative research in science education has uncovered many nave or incorrect ideas about aspects of science commonly held by students and others at all levels. This article discusses how misconceptions can cluster and compound. Robinson, William R. J. Chem. Educ.1998, 75, 1074.

Covalent Bonding |

Ionic Bonding

Demonstrations on Paramagnetism with an Electronic BalanceAdolf CortelThe demonstration shows the paramagnetism of common inorganic compounds by measuring the force with which they are attracted by a magnet over the plate of an electronic balance. Cortel, Adolf. J. Chem. Educ.1998, 75, 61.

Magnetic Properties |

Atomic Properties / Structure |

Covalent Bonding

Teaching Chemistry with Electron Density ModelsGwendolyn P. Shusterman and Alan J. ShustermanThis article describes a powerful new method for teaching students about electronic structure and its relevance to chemical phenomena. This method, developed and used for several years in general chemistry and organic chemistry courses, relies on computer-generated three-dimensional models of electron density distributions.Shusterman, Gwendolyn P.; Shusterman, Alan J. J. Chem. Educ.1997, 74, 771.

Visualization of the Abstract in General ChemistryPaselk, Richard A.A series of software programs for beginning chemistry, including a series of modules addressing the fundamental phenomena associated with bonding, the microscopic phenomena underlying commonly observed systems, and a reference periodic table.Paselk, Richard A. J. Chem. Educ.1994, 71, 225.

Bond energies in the interpretation of descriptive chemistryHowald, Reed A.Most of the discrepancy between bond energies and bond dissociation energies is eliminated by the inclusion of pi bonding effects and using bond energies referred to as hypothetical "valence state" atoms in those cases where spin pairing provides substantial stabilization for the free atom.Howald, Reed A. J. Chem. Educ.1968, 45, 163.

General chemistry exercise using atomic and molecular orbital modelsWalker, Ruth A.Styrofoam balls and pipecleaners are used to construct models designed to convey an understanding of the three-dimensionality of the electron distribution in the ground state atom and the effect of bonding on this distribution.Walker, Ruth A. J. Chem. Educ.1965, 42, 672.

The chemistry of the noble gasesHyman, Herbert H.Summarizes the chemistry of the noble gases and their bond-forming abilities.Hyman, Herbert H. J. Chem. Educ.1964, 41, 174.

Gases |

Main-Group Elements |

Covalent Bonding

Principles of chemical reactionSanderson, R. T.The purpose of this paper is to examine the nature of chemical change in the hope of recognizing and setting forth the basic principles that help us to understand why they occur.Sanderson, R. T. J. Chem. Educ.1964, 41, 13.

Non-existent compoundsDasent, W. E.The purpose of this review is to examine compounds that do not violate the rules of valence but which are nevertheless characterized by a high degree of instability, and to consider why these structures are unstable or non-existent.Dasent, W. E. J. Chem. Educ.1963, 40, 130.

Molecular models: A general chemistry exercisePierce, James B.Students are provided a list of bond angles, covalent radii, and van der Waals radii, and sufficient polystyrene spheres, and then asked to construct models of molecules and ions.Pierce, James B. J. Chem. Educ.1959, 36, 595.